Manufacture of metal fluorides



MayI 23, 19-61 R. E. FREDRICKSON ET AL MANUFACTURE OF METAL FLUORIDES Filed Jan. '7, 1957 f Make-0,0 Mg 672 NaOH nited States Patent MANUFACTURE F METAL FLUORIDES Robert E. Fredrickson, Lake Jackson, William A. Mod, Freeport, and Bob R. Harrell, Lake Jackson, Tex., assignors to The Dow Chemical Company, Midland, Mich., a corporation of Delaware Filed Jan. 7, 1957, Ser. No. 632,720

18 Claims. (Cl. 23-88) This invention relates to an improved process for preparation of metal iiuorides.

In recent years the demand for metal iluorides has increased considerably. Industry with the present methods of manufacturing these iluorides has been slow in meeting this growing demand. The majority of `the processes used for the preparation of the uorides require expensive specialized equipment, because hydrogen iluoride is used. Since these processes depend upon hydrogen fluoride production, the preparation of these salts is expensive and the ability of the industry to expand rapidly to meet the demand is greatly limited. To overcome these disadvantages, a number of processes have been described whereby metal uorides can be made without the use of hydrogen lluoride. By these methods it is practically impossible to produce metal iluorides free from other reaction products due to separation diiculties. These processes are not adaptable for preparation of metal iluorides for general use and are limited to the manufacture of metal fluorides for a particular purpose where the impurities are not detrimental. A process wherein easily recoverable metal iluorides, suitable for general use, could be made without depending upon the production of hydrogen fluoride would aid in meeting the growing demand for relatively pure metal uorides.

According to the invention, easily recoverable metal uorides are economically manufactured by reacting calcium uoride with magnesium chloride to prepare magnesium uoride and reacting the magnesium iluoride with a strongly alkaline metal hydroxide to form the metal fluoride. Also magnesium hydroxide is produced `which can be reacted with hydrogen chloride to form additional magnesium chloride which may be recycled. 'The reactions involved in this process may be illustrated by the following formulae:

4where in Equation 2 M is a metal forming a strongly alkaline hydroxide and n is the valence of the metal M, either 1 or 2.

In the improved process of the present invention, 'hydrogen fluoride is not used. Since relatively expen- -sive equipment is not required, the production of the uoride can be readily increased whenever there is a ydemand. The uorides made by the process can be -easily separated in crystalline state from the reaction iproducts by classication. Usually, since the product is obtained in a crystalline state, further purification is `not necessary to make the product satisfactory for com- 'mercial use. In this process dilute solutions of the Ialkaline hydroxide can be used. With the exception of potassium hydroxide, impurities in the dilute solutions, such as those found in an eluent of an electrolytic chlorine cell, do not materially affect the purity or the reycovery of the uoride product. The ability to use these ice 2 available dilute impure solutions is particularly advantageous economically.

The new improved process can be used for manufacturing fluorides of any metal which forms a strongly alkaline hydroxide, such as, for example, sodium, potassium, lithium, barium, strontium, etc. lIt is possible to manufacture the metal uorides by using only the reactions indicated by the first two equations. However, the economy of the process is considerably improved by combining the third reaction with the rst two. Relatively pure metal iuorides are made by utilizing the physical characteristics of the magnesium lluorideand magnesium hydroxide precipitates to effect the separations of these precipitates by a mechanica-l means from the liquid and other solids in the reaction mixtures. By reacting calcium uoride from sources, such as uorspar, with magnesium chloride under specied conditions, a precipitate of magnesium uoride is obtained which can be easily separated from any unreacted calcium fluoride or solid inerts present as well as from the remaining solution. In the reactions of magnesium fluoride with alkaline metal hydroxides, the metal fluorides obtained, with the exception of potassium iluoride, have a relatively low solubility in the reaction products. They are crystalline in form and are readily separable from the magnesium hydroxide and the other reaction products. With metal uorides which are soluble, such as potassium fluoride, the solution of the uoride is recovered by ltration and th'en further processed, as by evaporation, to obtainY the free salt.

In describing the process, the individual reactions will be rst discussed and then an application of the process to the preparation of sodium fluoride as shown diagrammatically by the attached drawing will be described.

In reacting the magnesium chloride with calcium uo ride, a magnesium chloride solution containing not greater than 30 weight percent of magnesium chloride must be used in order to obtain a magnesium iluoride precipitate which can be separated from the reaction mixture.. To effect the separation, it is necessary to obtain a precipitate which can be easily separated from the solids in the reaction mixture and still be readily filterable to recover it from the resulting calcium chloride solution. Dilute solutions of magnesium chloride will give a magnesium uoride product which is more readily separable than the product obtained with more concentrated solutions. As the concentration of the magnesium chloride solution used is increased, the precipitate of magnesium uoride obtained has a greater tendency to adhere to inert solids in the reaction mixture and also to form a more impervious til-ter cake. The eiect of the concentration of the magnesium chloride solution in producing the diicultly separable form of magnesium fluoride is only gradual when the concentration is increased from around l() to 28 percent. At concentrations above 28 percent, a small increase in the concentration will profoundly affect the magnesium uoride product obtained making it impractical to use a concentration containing more than 30 weight percent magnesium chloride. Further, attempts to obtain a high conversion of calcium fluoride with solutions greater than 30 Weight percent may result in obtaining a cement-type product which adheres to the walls of the reactor and can only be removed by chipping.

Since in the reaction of calcium fluoride from sources, such as fluorspar, the unreacted calcium uoride is discarded with the reaction mixture solids, a high conversion of calcium uoride is desirable. The conversion o'f calcium fluoride depends upon the reaction temperature 'and the excess of magnesium chloride used. A high reaction temperature in the range of 200 to 270 C., preferably around 250 C., is generally employed to obtained these 3 N. high conversions of the calcium fluoride without having to'use an unduly large excess of magnesium chloride.

Although a more easily separable product is obtainedv with the more dilute solutions of magnesium chloride, a greater excess of this solution is required. Thus, a'pracu- Vcal lower limit o'f the magnesium chloride solutions that may be employed is around l weight percent. With solutions in the range of l0 to 30 weight percent of r11agnes'ium chloride, preferably in the range of 18 to 22 weight 75 to 80 percent are obtained.

Since the reaction is carried out in an aqueous medium at temperatures in the range of 230 to 270, sufcient pressure must be used to maintain themixture in liquid phase. temperatures, a pressure in the range of 450 to 800 pounds per square inch is generally required.

The reaction time necessary to'obtain a substantially complete conversion of the calcium fluoride in the lfluorspar depends upon the particle size of the lluorspar used in, the reaction. The uorspar is usually ground to pass through a 200 mesh screen, which permits a goo'd contact of the calcium fluoride with the'magnesium chloride in the reaction slurry, and requires a reaction time of from l to 30 minutes to substantially convert all of the calcium uoride. When the fluorspar is not ground Ato as line a particle size, a longer reaction time is required.

While o'ther mechanical methods may be used to efrect the separation of magnesium fluoride fromythe reaction products, generally the magnesium uoride is Separated n from the inerts and other solids present in the Vreacted mixture by elutriation and recovered from the calcium chloride solution by settling and ltration.

The reaction of magnesium uoride With the alkaline hydro'xide can be carried out in a stirred reactor under atmospheric pressure. For the reactions of the alkaline hydroxide which will form metal fluorides insoluble in the reaction mixture, at least a stoichoimetric amount of magnesium fluoride must be used in order to obtain a practical conversion of the magnesium uo'ride. Preferably, a 50 to 200 percent stoichiometric excess of magnesiurn iiuoride is used. When slightly less than stoichiometric amounts are used, less than 1/2 of the alkaline hydroxide will react. With a stoiehiometric amount of magnesium liuoride, around 60 percent of the hydroxide will be converted, while with a 50 percent stoichiometric excess, 88 percent, and with a 200 percent excess, 98 percent conversion is obtained. With alkaline hydroxides which will form metal iiuorides soluble in the reaction mixture, such as potassium liuoride, at least a stoichiometric amount of the hydroxide is required. It is preferred to use a stoichiometric excess of the hydroxide in the range of 50 to 150 percent instead of an excess of magnesium fluoride.V With the excess hydroxide substantially complete conversion of the magnesium uoride to the metal uoride can be obtained.

Although the concentration of the alkaline hydroxide p used is not critical, it is preferred to use a solution containing at least 8 percent by `Weight of the hydroxide. In the manufacture of metal lluorides which are insoluble in the reaction mixture, a relatively impure hydroxide may be used, for example, in the preparation o'f sodium linoride, etliuent from an electrolytic cell is satisfactory. It isf preferred to use a relatively pure Valkaline hydroxide for the preparation of metal liuorides which are soluble, such as potassium fluoride, since any impurities in the hydroxide will `be with the metal uoride in the solution portion o'f the reacted mass and this may make it more diflicult to recover a relatively pure product from the solution. The reaction between the alkaline hydroxide and the magnesium fluoride maybe carried out at a To keep the water from vaporizing `at theseV 4A temperature between l40 C. and the boiling point of the mixture, the optimum temperature being inthe range of around to 90 C. The reaction between the reactants is substantially complete in about l to 3 hours.

Separation of the metal tluorides from the magnesium hydroxide and the unreacted magnesium liuoride is readily accomplished. With the exception of potassium iiuoride, the solubility of the metal fluoride is relatively low and crystals of the iluoride are formed which may be separated from the magnesium compounds by elutriation. The crystals may then be centrifuged, washed, and dried. The magnesium hydroxide and the unreacted magnesium filuoride can be concentratedl in another settler and the underflow filtered to recover the magnesium compounds.`

Where the fluoride is soluble such as potassium fluoride, the metal uoride solution portion of the reaction mass may be 'separated from the insoluble part by settling and filtration. The solution can then be evaporated to recover the fluoride salt by crystallization.

The magnesium hydroxide recovered from the above step may be neutralized with hydrochloric acid to convert the magnesium hydroxide to magnesium chloride. Unreaeted magnesium fluoride which may be present is Vnot adversely affected by the neutralization and may be separated from the resulting magnesium chloride solution by filtration and recycled back to the alkaline hydroxide reaction, if desired. Magnesium chloride obtained Vin the neutralization step may be recycled back to the rst step to be reacted with more iiuorspar. The solution obtained in this step is relatively dilute and may be used directly without further concentration or dilution, if desired. Y

The process may be more fully understood by referring to the accompanying drawing which illustratesV diagrammatically an application of the improved process for manufacture of Sodium iluoride.

Ground'liuorspar and an aqueous magnesium chloride solution are added to blend tank l where theV constituents are mixed by an agitator. From tank 1, the slurry is pumped to reactor 2. In thereactor the mixture is heated to a temperature from 230 to 270 C. under suiiicient pressure to prevent substantial vaporization of the water present and reacted for about l5 to 30'mi'nutes. From reactor 2, the reacted slurry is `discharged to flash ytank 3 where the pressure'on the constituents Vis reduced to atmospheric pressure. The reduction in pressure will result in the Vaporization of the water cooling the products before their introduction into classifier 4. To have a continuous process, a continuous reactor or more than one reactor may be used so that a continual flow to classifier 4 can be maintained. In classifier 4, the cal cium chloride solution and the magnesium fluoride are separated from the inerts which were in the liuorspar by elutriation. The solids settle to the bottom of tank 4 and are discharged as underow through line 26. The calcium chloride and the magnesium fluoride precipitate leave classifier 4 in the overflow and pass through line 22 to settling tank 5. In tank S, the magnesium fluoride precipitate settling to the bottom is withdrawn through line 23 and recovered by ltering and washing in filter 6. The calcium chloride solution is removed from the settling tank as an overilow and discharged to waste with the filtrate from the filter. Some of the calcium chloride solution is recycled by line 25 to the bottom of classilier 4 where it provides the upward liow for the elutriation. The reaction of magnesium uoride with sodium hydroxide is carried out in reactor 7. When the desired amount of magnesium iiuoride has been recovered by filter 6, it is introduced into reactor 7. The hydroxide containing about Sto l0 percent by weight of sodium hydroxide is fed to the reactor. Thereactants are agitated and reacted at 80 C. for alength of time of l to 3 hours. The eiuent from reactor 7 is dischargedthrough line 31 to classifier 9 where by using elutriation the sodium liuo ride crystals settleto the bottom ot the tank to be re 'gesamte oved as underfiovv. These crystals may then be further processed by centrifuging, washing, and drying. The magnesium hydroxide, the unreacted magnesium fluoride, and the remaining solution are removed as overflow and passed through line 32 to settling tank 10. The magnesium hydroxide and the unreacted magnesium fiuoride settle to the bottom of tank and are withdrawn through line 33 as a slurry to be filtered in filter 13. Part of the solution removed as overflow from settling tank 10 is recycled through line 34 to provide the upward flow for the elutriation in classifier 9, while the remaining overflow with the filtrate from filter 13 is discharged to waste or to further processing to recover the small amount of the metal fluoride dissolved in the solution.

The magnesium hydroxide and the unreacted magnesium fluoride from filter 13 is charged to neutralization tank 14 to which suliicient amount of hydrochloric acid is added to neutralize the magnesium hydroxide. The efiiuent from the neutralizer is passed lto filter 15 where the magnesium fluoride is separated from the magnesium chloride solution and returned to reactor 7. The magnesium chloride solution obtained is recycled to blend tank 1 where it can be intermixed with more fluorspar to be reacted.

It is evident that this improved process may be applied in other ways than shown by the drawing. Different types of equipment may be employed and the separation of the products may be made by other methods.

The following examples further illustrate the invention but are not to be construed as limiting the invention thereto.

Example I A series of runs were made Where magnesium chloride was reacted with fluorspar in a 1 liter pressure reactor equipped with an agitator. The concentration and amount of the magnesium chloride solution used were varied with each run. The reactions were carried out at a temperature of 250 C. and under sufiicient pressure to maintain the reaction mixture in liquid phase. Pressure employed varied with the concentration of the magnesium chloride solution used and was in the range of 450 to 600 pounds per square inch.

In the runs, the reactor was charged with 10() grams of fiuorspar, ground to pass through a 200 mesh screen and containing 97.7 weight percent of calcium fluoride, and with the magnesium chloride solution. The resulting slurry was agitated, heated to 250 C., and maintained at this temperature for minutes. Then it was cooled, filtered, and washed. The filtrate and the wash water were combined and the solution analyzed for calcium from which the calcium fiuoride conversion was determined. Results obtained are shown in the table below.

l The magnesium fluoride obtained from the run using a percent stoichiometric excess of a magnesium chloride solution containing l5 weight percent of magnesium chloride was reacted with effluent from an electrolytic chlorine cell containing 8.7 weight percent of sodium hydroxide. A series of runs were made at atmospheric pressure using different ratios of the reactants.

In the runs, 362 grams of the chlorine cell eiuent was added to a stirred reactor. For each run a different amount of magnesium fluoride was also added to the reactor in form of a dry filter cake containing l97 weight percent of magnesium fiuoride. The mixture was heated to 68 C. and maintained at lthis temperature for 2 hours. Then it was filtered to separate the solids. The filtrate was analyzed for sodium hydroxide and the conversion of the hydroxide was calculated. Results obtained are given in the table below:

Percent Moles of MgFg per mole of NaOH Conversion of NaOH to NaF Example II Barium hydroxide was reacted with magnesium fluoride in a closed glass reactor equipped with a stirrer.l

To the reactor were added 100 grams of a 10 percent by weight of barium hydroxide aqueous slurry and 3.6 grams of a filter cake containing percent by weight of magnesium uoride and the remainder water. The mixture was heated to about 80 C. and reacted at this temperature for l hour. The resulting mixture was filtered while hot. Analysis of the filtrate and residue showed that 54.5 percent of the magnesium fluoride was converted to barium fluoride.

Example III A run was made similar to the one described in EX- ample II except that lithium hydroxide was reacted in placed of barium hydroxide. To the reactor were added grams of water, l0 grams of lithium hydroxide, and 13 grams of magnesium fluoride. The mixture was reacted at 90 for `one hour and the resulting slurry was filtered while hot. Analysis of the filtrate show that 71 percent of the magnesium liuoride was converted to lithium fluoride. Y

Example V A series of runs were made in a manner similar to that described in Example II. In the runs different amounts of potassium hydroxide was reacted with a given amount of magnesium fluoride.

To the reactor, 2l grams of a dry filter cake containing 97 weight percent of magnesium uoride and a 10 weight percent potassium hydroxide were added. The mixture was heated to 90 C., reacted for 3 hours, and filtered while hot. The filtrate was analyzed to determine the percent of magnesium fluoride converted to potassium fluoride.

The results obtained are given below:

Percent Conversion of Magnesium Fluoride Stoichiometric Ratio of KOH to MgFg Woo Example VI AI semi-continuous process similar to the one shown by thejattached drawing was used in the preparation of 'sodium uoride..

To a l liter pressure reactor equipped With an agitator, 100, grams of uorspar containing 97.7 weight percent of calcium uoride and 662 grams of an aqueous magnesium chloride solution containing 22 weight percent of magnesium chloride Were added. The reactants were heated to 250 C. under` a 600 pounds per square inch gauge pressure and reacted for 20 minutes.

After the reacted mass was cooled, the magnesium uoride and calcium chloride solution were separated from the inerts of the tluorspar by elutriation'in a laboratory settler. Thelaboratory settler consisted of a 7/s inch I.D. tube which at the top was divergingly enlarged to 51/2 inch I.D. vArrupvvard owrate ofV 3.06gallons per minute of the calcium chlorideY solution per square foot of cross sectional area was employed.

The magnesium lluoride product was separated from the calcium chloride solution by ltration, Washed, and dryed. The product contained 97 weight percent of magnesiumhuoride., Analysis of the filtrate for calcium iudicatedthat 98 percentof the calcium-,fluoride in the uorspar has been converted to magnesium fluoride.

The magnesium Vfluoride productobtained was placed in an open flask. Also, some recycle magnesium fluorideobtained in a previous run was added to give a total of. 150 gramsof magnesium fluoride. Thiscombined product was mixed with 1100 grams of an electrolytic chlorine cell eluent containingf 8.7 Weightpercent of sodum hydroxide, and reacted, at 60 C. for 3 hours.

Separation of the resulting sodium lluoride fromthe magnesium hydroxide andthe excess Vmagnesium lluoride was effected in a settler consisting of a 21/2` inch LD. tube. An upward flow rate in the settler of 4.4 gallons per4 minute of the. filtrate from the overflow` per square foot of cross sectional area was used. Analysis of the filtrate indicatedthat 98 percent of the sodium hydroxide was convertedrto sodium uoride.

Thermagnesium hydroxide andthe excessmagnesium fluoride obtained in the overow were reacted for one hour at room temperature With 439 grams of a hydrochloric acid solution containing 20 Weight percent of hydrogen chloride. The resulting magnesium chloride was recycled tobe reacted with more fluorspar and the magnesium fluoride was recycled to be reacted with more sodium hydroxide in a following run.

What is claimed is:

1. lA process for the preparation of a metal fluoride from calcium fluoride, which comprisesintermixing the calcium fluoride with an. aqueous solutionof magnesium chloride containing in the range of from 10 to30 Weight percent magnesium chloride to-form a slurry, heating the slurry at a temperature in therange of 200 to,270. C. undery sufficient pressure to prevent substantial vaporization of water from the slurry Vso as to convert the calcium uoride to calcium chloride and the Amagnesium chloride tomagnesilnnouoridq separating the magnesium fluoride fromhthe calcium chloride and inerts interrnixing the recovered magnesium fluoride with a hydroxide selected from the group consisting of sodium hydroxide, lithium hydroxide, potassium hydroxide, strontium `hydroxide and `barium hydroxide to convert lthe magnesium fluoride and the hydroxide to magnesium hydroxide and a metal uoride, and recovering the. metal fluoride from `the reacted mixture.

2. A process for the preparation of a metal uoride from iluorspar, which comprises intermixing ground fluorspar with a l5 to 25 percent stoichiometric excess of an aqueous magnesium chloride solution containing from lO'to 30 weight percent magnesium chloride to form a slurry, heating the slurry at a temperature inthe range of 200 to 270 C. -under sui'hcient'pressure to prevent'sun- Vstantial vaporization of Water from the slurry so as to convert the calcium-fluoridein the uorspar-to-calcium chloride and the magnesium chloride to magnesium uoride, separating the magnesium fluoride from the calcium chloride and inerts, intermixing the recovered magnesium lluoride with a hydroxideselected from the group consisting of sodium hydroxide, a lithium hydroxide, barium hydroxide, and strontium hydroxide, to convertv the magnesium uoride and the hydroxidek to magnesium hydroxide and a metal fluoride, and recovering the metal fluoride from the reacted mixture.

3. A process for the preparation of a metal iluoride from fluorspar, which comprises intermixing ground fluorspar with a k15 to 25 percent stoichiometric excess of an aqueous magnesium chloride solution containing from l0 to 30 Weight percent magnesium chloride to form a slurry, heating the slurry at a temperature in the range of 200 to 270 C. under sucient pressuretoprevent substantial vaporization ofwater from the slurry so as to convert the calcium fluoride in the fluorspar to calcium chloride and the magnesium chloride tov magnesium lluoride, separating the magnesium uoride fromthe. calcium chloride and inerts, intermixing the recovered magnesium lluoride with a hydroxide selected from theY group consisting of sodium hydroxide, lithium hydroxide,` barium hydroxide, and strontium hydroxide, in proportions such that the amount of magnesium fluoride is inl the range of a stoichiometric amount to a 200 percent stoichiometric excess tov convert the magnesium fluoride and the hydroxide toV magnesium hydroxide and a metal uoride, re- .covering the metal uoride from the reacted mixture, separating the magnesium hydroxide and the unreacted magnesium uoride from the metal uoride-free reaction mixture, vadding hydrochloric acid to the separated magnesium hydroxide and unreacted magnesium fluoride to convert the magnesium hydroxide to a magnesium chloride solution, separating the unreacted magnesium fluoride from the resulting magnesium chloride solution, returning the magnesium lluoride to be intermixed withV additional hydroxide, and returning the resulting magnesium chloride solution to be mixed with more uorspar.

4. A process -for theV preparation of a metal fluoride from .iluorspan which comprises intermixing ground lluorspar with a l5 to 25 percent stoichiometric excess of an aqueous magnesium chloride solution containing from 18 to 22. weight percent magnesium chloride to Vforrn a slurry, heating the slurry at a temperature of around 250 C. under `suicient pressure to prevent substantial vaporization of Water from the slurry so as to convert the calcium fluoride in the fluorspar to calcium chloride and the magnesium chloride to magnesium uoride, separating the magnesium fluoride from the calcium chloride and inerts, intermixing the recovered magnesium lluoride in a 50 to 200 percent stoichiometric excess Ywith an aqueous solution containing at least 8 percent by weight of a hydroxide selected from the group consisting fo sodium hydroxide, lithium hydroxide, barium hydroxide, and strontium hydroxide at a temperature between 40 C. and the boiling point of the mixture to react the magnesium fluoride and the hydroxide to form magnesium hydroxide and a metal. fluoride, recovering the metal fluoride from the reacted mixture, sepiaratingtheY magnesium hydroxide and the unreacted magnesium vfluoride from the metal uoride-iree reaction mixture, adding hydrochloric acid to the separated magnesium hydroxide and magnesium fluoride to convert the magnesiumY hydroxide topa magnesium chloride solution, separating the unreacteed magnesium fluoride from the` magnesium chloride solution, returning the magnesium fluoride vto be intermixed with additional hydroxide, and returning Vthe resulting magnesium chloride solution to be mixed with more -iluorspan 5. A process for the preparation of a metal fluoride from fluorspar, which comprises intermixing ground iluorspar witha 15 to x25 percent stoichiometricexcess of an aqueous magnesium chloride solution containing ff acentos the calcium fluoride in the fluorspar to calcium chloride and the magnesium chloride to magnesium fluoride, separating the magnesium uoride from the calcium chloride and inerts, intermixing the recovered magnesium iluoride in a stoichiometric excess in the range of 50 to 200 percent with Ian aqueous solution containing at least 8 percent by weight of a hydroxide selected from the group consisting of sodium hydroxide, lithium hydroxide, barium hydroxide, and strontium hydroxide at a temperature in the range of 80 to 90 C. to react the magnesium fluoride and the hydroxide to form magnesium hydroxide and a metal fluoride, recovering the metal fluoride from ther eacted mixture, separating the magnesium hydroxide and the unreacted magnesium uoride from the metal uoride-free reaction mixture, adding hydrochloric acid to the separated magnesium hydroxide and magnesium uoride to convert the magnesium hydroxide to a magnesium chloride solution, separating the unreacted magnesium uoride from the magnesium chloride solution, returning the magnesium fluoride to be intermixed with additional hydroxide, and returning the resulting magnesium chloride solution to be mixed with more uorspar.

6. A process `according to claim wherein the hydroxide is sodium hydroxide.

7. A process yaccording to claim 5 wherein the hydroxide is lithium lhydroxide.

8. A process according to claim 5 wherein the hydroxide is barium hydroxide.

9. A process according to claim 5 wherein the hydroxide is strontium hydroxide.

10. A process `for the preparation of potassium uoride from calcium fluoride, which comprises intermixing calcium fluoride with a 15 to 25 percent stoichiometric excess of an aqueous magnesium chloride solution containing from to 30 weight percent magnesium chloride to form a slurry, heating the slurry at a temperature in the range of 200 to 270I C. under sulicient pressure to prevent substantial vaporization of water from the slurry so as to convert the calcium fluoride in the uorspar to calcium chloride and the magnesium chloride to magnesium fluoride, separating the magnesium fluoride from the calcium chloride and inerts, intermixing potassium hydroxide with the recovered magnesium fluoride to convert the magnesium iluoride and the potassium hydroxide to magnesium hydroxide and a potassium iluorid-e solution, separating the potassium iluoride solution from the magnesium hydroxide, and recovering the potassium uoride from the solution.

11. A process for the preparation of potassium uoride from fluorspar, which comprises intermixing ground uorspar with a to 25 percent stoichiometric excess of an aqueous magnesium chloride solution containing from 10 to 30 weight percent magnesium chloride to form a slurry, heating the slurry at a temperature in the range of 200 to 270 C. under sucient pressure to prevent substantial vaporization of Water from the slurry so as to convert the calcium fluoride in the uorspar to calcium chloride and the magnesium chloride to magnesium iiuoride, separating the magnesium uoride from the calcium chloride and inerts, intermixing potassium hydroxide with the recovered magnesium uoride to react the magnesium uoride with the potassium hydroxide to form magnesium hydroxide and a potassium tluoride solution, separating the potassium iiuoride so1ution from the magnesium hydroxide, recovering the potassium iluoride from the solution, adding hydrochloric acid to the magnesium hydroxide to convert the magnesium hydroxide to `a magnesium chloride solution, and returning the magnesium chloride solution to be intermixed with more uorspar.

12. A process-.flor the preparation of potassium uoride 'from' uo'rspar, which, GODJprises "intermixi' ng ground uorspar with a 15 to 25 percent stoichiometric excess of an aqueousmagnesiu'm chloride solution containing from 18 to 22 percent `by weight of magnesium chloride to form a slurry, heating the'slurr'y ata temperature of 200 to 270 C. under suih'cien't pressure to prevent substantial vaporization of water from the slurry so as to convert the calcium uoride in the fluorspar to calcium chloride and the magnesium chloride to magnesium tiuoride, separating the magnesium uoride from the calcium chloride and inerts, intermixing the recovered magnesium iluoride with a stoichiometric excess in the range of 50 to 150 percent of an aqueous solution containing at least 8 percent by weight of potassium hydroxide at a tempera-- ture between 40 C. and a boiling point of the mixtureto react the magnesium uoride with the potassium hydroxide to form magnesium hydroxide and a potassium uoride solution, separating the potassium fluoride solution from the magnesium hydroxide, recovering the p0- tassium uoride from the solution, adding hydrochloric acid to the magnesium hydroxide to convert the magnesium hydroxide to a magnesium chloride solution, and returning the magnesium chloride solution to be mixed with more iiuorspar.

13. A process for the preparation of potassium iiuoride from iluorspar, which comprises intermixing ground uorspar with a l5 to 25 percent stoichiometric excess of an aqueous magnesium chloride solution containing from 18 to 22 percent by weight of magnesium chloride to form a slurry, heating the slurry at a temperature of 250 C. under suiiicient pressure to prevent substantial vaporization of water from the slurry so as to convert the calcium uoride in the uorspar to calcium chloride and the magnesium chloride to magnesium uoride, separating the magnesium fluoride from the calcium chloride and inerts, intermixing the recovered magnesium fluoride with a stoichiometric excess in the range of 50 to 150 percent of an aqueous solution containing at least 8 percent by weight of potassium hydroxide at a temperature in the range of to 90 C. to react the magnesium fluoride with the potassium hydroxide to form magnesium hydroxide and a potassium fluoride solution, separating the potassium fluoride solution from the magnesium hydroxide, recovering the potassium uoride from the solution, adding hydrochloric acid to the magnesium hydroxide to convert the magnesium hydroxide to a magnesium chloride solution, and returning the magnesium chloride solution to be mixed with more fluorspar.

14. A process for the preparation of a metal uoride which comprises intermixing magnesium uoride in a stoichiometric excess in the range of 50 to 200 percent with an aqueous solution containing at least 8 percent by weight of a hydroxide selected from the group consisting of sodium hydroxide, lithium hydroxide, barium hydroxide, and strontium hydroxide at a temperature in the range of 80 to 90 C. to react the magnesium uoride and the hydroxide to form magnesium hydroxide and the metal uoride, and recovering the metal uoride from the reacted mixture.

15. A process according to claim 14 wherein the hydroxide is sodium hydroxide.

16. A process according to claim 14 wherein the hydroxide is lithium hydroxide.

17. A process according to claim 14 wherein the hydroxide is 'barium hydroxide.

18. A process according to claim 14 wherein the hydroxide is strontium hydroxide.

References Cited in the file of this patent UNITED STATES PATENTS 2,398,743 Heath et al Apr. 16, 1946 2,690,430 Anderson Sept. 28, 1954 (Other references on following page) 

1. A PROCESS FOR THE PREPARATION OF A METAL FLUORIDE FROM CALCIUM FLUORIDE, WHICH COMPRISES INTERMIXING THE CALCIUM FLUORIDE WITH AN AQUEOUS SOLUTION OF MAGNESIUM CHLORIDE CONTAINING IN THE RANGE OF FROM 10 TO 30 WEIGHT PERCENT MAGNESIUM CHLORIDE TO FROM A SLURRY, HEATING THE SLURRY AT A TEMPERATURE IN THE RANGE OF 200* TO 270*C. UNDER SUFFICIENT PRESSURE TO PREVENT SUBSTANTIAL VAPORIZATION OF WATER FROM THE SLURRY SO AS TO CONVERT THE CALCIUM FLUORIDE TO CACIUM CHLORIDE AND THE MAGNESIUM CHLORIDE TO MAGNESIUM FLUORIDE, SEPARATING THE MAGNESIUM FLUORIDE FROM THE CALCIUM CHLORIDE AND INTERS, INTERMIXING THE RECOVERED MAGNEISUM FLUORIDE WITH A HYDROXIDE SELECTED FROM THE GROUP CONSISTING OF SODIUM HYDROXIDE, LITHIUM HYDROXIDE, POTASSIUM HYDROXIDE, STONTIUM HYDROXIDE AND BARIUM HYDROXIDE TO MAGNESIUM FLUORIDE AND THE HYDROXIDE TO MAGNESIUM HYDROXIDE AND A METAL FLUORIDE, AND RECOVERING THE METAL FLUORIDE FROM THE REACTED MIXTURE. 